To find the mass of the iron compound required per tablet, we need to determine the molar mass of FeSO4路7H2O and use the stoichiometry to calculate the mass of FeSO4路7H2O that provides 50mg of iron(II).
Here's how we can do it step by step:
Step 1: Find the molar mass of FeSO4路7H2O.
To calculate the molar mass of FeSO4路7H2O, we need to sum up the atomic masses of all the elements in the compound.
Atomic masses:
- Fe: 55.845 g/mol
- S: 32.06 g/mol
- O: 16.00 g/mol (there are four oxygen atoms in FeSO4路7H2O)
- H: 1.00784 g/mol (there are 14 hydrogen atoms in FeSO4路7H2O)
Molar mass of FeSO4路7H2O:
= (55.845 g/mol) + (32.06 g/mol) + 4(16.00 g/mol) + 7(1.00784 g/mol)
= 278.04176 g/mol
Step 2: Calculate the mass of FeSO4路7H2O required per tablet.
Since the molar mass is given as grams per mole, we can use it to convert 50mg of iron(II) to the corresponding mass of FeSO4路7H2O.
Number of moles of iron(II) = Mass of iron(II) / Molar mass of Fe(II)
= 50 mg / (55.845 g/mol)
= 0.893 mol (approx.)
From the balanced chemical equation, we know that 1 mole of FeSO4路7H2O yields 1 mole of Fe(II). Therefore, the molar ratio of FeSO4路7H2O to Fe(II) is 1:1.
Hence, the mass of FeSO4路7H2O required per tablet would also be approximately 50mg.
Thus, approximately 50mg of the iron compound FeSO4路7H2O is required per tablet to provide the desired amount of 50mg of iron(II).